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Chapter 8: Problem 104

Although exact isotopic masses are known with great precision for most elements, we use the average mass of an element's atoms in most chemical calculations. Explain.

Short Answer

Expert verified
We use the average mass of an element's atoms in most chemical calculations because it provides a more accurate representation of the naturally occurring mixture of isotopes and simplifies calculations by using a single value. Although using exact isotopic masses might offer higher precision in some cases, the complexity added may not justify the marginal precision increase. Using the average atomic mass is a practical balance between accuracy and ease of use.

Step by step solution

01

Understanding Isotopes

Isotopes are atoms of the same element with different numbers of neutrons in their nuclei. This implies that these atoms have the same number of protons (and hence the same atomic number) but different atomic masses, determined by the sum of protons and neutrons in the nucleus. Since isotopes of an element have different masses, using the mass of a single isotope would not represent the entire element.
02

Calculating Average Atomic Mass

The average atomic mass of an element is calculated based on the relative abundances and masses of the element's natural isotopes. The average atomic mass is determined by multiplying the mass of each isotope by its relative abundance (as a fraction), and then summing up the results. Mathematically, the average atomic mass (A) can be represented by the formula: \(A = \sum_i (m_i a_i)\), where \(m_i\) is the mass of the i-th isotope, and \(a_i\) is the relative abundance of the i-th isotope.
03

Representativeness and Practicality

Since elements in nature often consist of a mixture of isotopes, using the average atomic mass in chemical calculations allows for more accurate and representative results. Additionally, using the average atomic mass simplifies calculations by providing a single value instead of considering each isotope separately. This makes it more practical for chemists to use in various calculations, such as determining the mass of reactants and products in a chemical reaction or calculating molar concentrations in solutions.
04

Precision vs. Simplicity

Even though using the exact isotopic mass might provide higher precision in some specific calculations, it may not be practical for most chemical calculations. In many cases, the difference between using exact isotopic masses and the average atomic mass might be negligible, and the additional complexity introduced may not justify the marginal increase in precision. Therefore, chemists choose to use the average atomic mass for most calculations as it provides a practical balance between accuracy and ease of use.

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Most popular questions from this chapter

Calculate the mass in grams of each of the following samples. a. 0.251 mol of ethyl alcohol, \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\) b. 1.26 mol of carbon dioxide c. \(9.31 \times 10^{-4}\) mol of gold(III) chloride d. 7.74 mol of sodium nitrate e. 0.000357 mol of iron

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